Book: MTS: 19

Question 1

Using stoichiometry and equilibrium problem-solving techniques to calculate the effect of added H3O+ or OH- on buffer pH.

Answer 1

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Question 2

Using the Henderson-Hasselbalch equation to calculate buffer pH.

Answer 2

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Question 3

Using molecular scenes to examine buffers.

Answer 3

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Question 4

Choosing the components for a buffer with a given pH and calculating their quantities.

Answer 4

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Question 5

Calculating pH at any point in an acid-base titration.

Answer 5

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Question 6

Choosing an appropriate indicator based on the pH at various points in a titration.

Answer 6

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Question 7

Writing K_sp expressions for slightly soluble ionic compounds.

Answer 7

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Question 8

Calculating a K_sp value from solubility data.

Answer 8

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Question 9

Calculating solubility from a K_sp value.

Answer 9

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Question 10

Using K_sp values to compare solubilities for compounds with the same total number of ions.

Answer 10

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Question 11

Calculating the decrease in solubility caused by the presence of a common ion.

Answer 11

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Question 12

Predicting the effect of added H3O+ on solubility.

Answer 12

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Question 13

Using ion concentrations to calculate Q_sp and compare it with K_sp to predict whether a precipitate forms.

Answer 13

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Question 14

Comparing K_sp values in order to separate ions by selective precipitation.

Answer 14

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Question 15

Calculating the equilibrium concentration of a hydrated metal ion after addition of excess ligand forms a complex ion.

Answer 15

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Question 16

Using an overall equilibrium constant (K_sp)(K_f) to calculate the effect of complex-ion formation on solubility.

Answer 16

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